The temperature of the water vapor (H,0) inside a pressure cooker increased from 295 K to 395 K. AS the sample is heated, the pressure of the water vapor went from 21.0 kPa to

P₂ = 28.12 KPa

Explanation:

Given data:

Initial temperature = 295 K

Final temperature= 395 K

Initial pressure = 21.0 KPa

Final pressure = ?

Solution:

According to Gay-Lussac Law,

The pressure of given amount of a gas is directly proportional to its temperature at constant volume and number of moles.

Mathematical relationship:

P₁/T₁ = P₂/T₂

Now we will put the values in formula:

21.0 KPa / 295 K = P₂/395 K

P₂ = 21.0 KPa× 395 K / 295 K

P₂ = 8295 KPa. K /295 K

P₂ = 28.12 KPa

n2(g) + 3h2-> 2nh3(g)   this is the balanced equation

note the mole ratio between n2, h2 and nh3.   it is 1 : 3 : 2   this will be important.

moles n2 present = 28.0 g n2 x 1 mole n2/28 g = 1 mole n2 present

moles h2 present = 25.0 g h2 x 1 mole h2/2 g = 12.5 moles h2 present

based on mole ratio, n2 is limiting in this situation because there is more than enough h2 but not enough n2.

moles nh3 that can be produced = 1 mole n2 x 2 moles nh3/mole n2 = 2 moles nh3 can be produced

grams of nh3 that can be produced = 2 moles nh3 x 17 g/mole = 34 grams of nh3 can be produced

note:   the key to this problem is recognizing that n2 is limiting, and therefore limits how much nh3 can be produced.

it's filtration, but this is an assumption so my apologies if i got this